Respuesta :
Answer : The pH of the solution is, 1.88
Explanation : Given,
[tex]K_a=1.1\times 10^{-2}[/tex]
Concentration of [tex]HClO_2[/tex] = 0.35 M
Concentration of [tex]NaClO_2[/tex] = 0.29 M
First we have to calculate the value of [tex]pK_a[/tex].
The expression used for the calculation of [tex]pK_a[/tex] is,
[tex]pK_a=-\log [K_a][/tex]
Now put the value of [tex]K_a[/tex] in this expression, we get:
[tex]pK_a=-\log (1.1\times 1-^{-2})[/tex]
[tex]pK_a=2-\log (1.1)[/tex]
[tex]pK_a=1.96[/tex]
Now we have to calculate the pH of the solution.
Using Henderson Hesselbach equation :
[tex]pH=pK_a+\log \frac{[Salt]}{[Acid]}[/tex]
[tex]pH=pK_a+\log \frac{[NaClO_2]}{[HClO_2]}[/tex]
Now put all the given values in this expression, we get:
[tex]pH=1.96+\log (\frac{0.29}{0.35})[/tex]
[tex]pH=1.88[/tex]
Therefore, the pH of the solution is, 1.88
